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Chapter 1 Dipoles, molecular polarity. Ways to Represent Polarity in Molecules H F electron rich region electron poor region  

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Presentation on theme: "Chapter 1 Dipoles, molecular polarity. Ways to Represent Polarity in Molecules H F electron rich region electron poor region  "— Presentation transcript:

1 Chapter 1 Dipoles, molecular polarity

2 Ways to Represent Polarity in Molecules H F electron rich region electron poor region  

3 Dipole Moment (  ) H F electron rich region electron poor region    = q x r magnitude of charge =  = |  | bond length moment in Debyes (D) 1 D = 3.36 x 10 -30 Coulomb. meter

4 Explain the Trend  EN drops

5 More Complex Molecules? Consider molecular shape (bond orientation) bond polarity lone pairs (and sometimes) atom size What is symmetry of e- distribution?

6 Consider NH 3 Lewis Structure Need # valence e- from all atoms Need bond arrangement (connectivity)

7 Consider NH 3 Lewis Structure # valence e- = 5 (N) + 1 (3H) = 8e- Three N-H bonds H - N - H | H..

8 Consider NH 3 From the Lewis structure Deduce e- pair geometry at central atom THEN find molecular geometry/shape Any predictions? H - N - H | H..

9 : :: : Consider NH 3 molecular shape individual bond dipoles lone pair “dipoles” 4e- pairs at N  tetrahedral e- pr geometry Lone pair at N  molecular geometry/shape is trigonal pyramidal

10 .. : :: : Which molecule is more polar? molecular shape individual bond dipoles lone pair “dipoles”

11 .. : :: : Which molecule is more polar?

12 .. : :: : Which molecule is more polar?

13 Attractions Between Dipoles  

14 E coulomb  q E coulomb  1/d

15 Dipole-Dipole Interactions Dipoles align,  + of one dipole to   of another Magnitude of attraction E coulomb  (  + )(   )/d Increases with dipole moment ~5-25 kJ/mol   …... d d

16 NOFNOF H..…NOFNOF Hydrogen Bonding: Special Type of Dipole-Dipole Attraction From another molecule From one molecule  Only applies to molecules with H bonded to N, O, or F  ~10-40 kJ/mol (larger than most dipole-dipole attractions)  ..… H bond

17 Why Are Hydrogen Bonds So Strong?  EN for H and N,O, F = very large, so N-H, O-H, F-H bonds are very polar (  +  -  are large) H atoms are small, so N, O, F of one molecule can closely approach H of another molecule (d is small) NOFNOF H … NOFNOF E coulomb  (  + )(   )/d H bond

18 Hydrogen Bonds in Water

19 Large Molecules Can Have Intramolecular Hydrogen Bonds

20 Hydrogen Bonds in Chitin


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